101. The molal elevation constant for water is 0.52 . What will be the boiling point of 2 molar sucrose solution at \(1 \mathrm{~atm}\) pressure? (Assume b.p. of pure water is \(100^{\circ} \mathrm{C}\) ) [AMU 2004]

1) \(101.04^{\circ} \mathrm{C}\)

2) \(100.26^{\circ} \mathrm{C}\)

3) \(100.52^{\circ} \mathrm{C}\)

4) \(99.74^{\circ} \mathrm{C}\) 102. Solution \(A\) contains \(7 \mathrm{~g} / \mathrm{L}\) of \(\mathrm{MgCl}_{2}\) and solution \(B\) contains \(7 \mathrm{~g} / \mathrm{L}\) of \(\mathrm{NaCl}\). At room temperature, the osmotic pressure of [Kerala CEE 2005]

1) 50

2) 180

3) 102

4) 25

5) 51

103. \(X\) is dissolved in water. Maximum boiling point is observed when \(X\) is ....(0.1 \(\mathrm{M}\) each) [DCE 2005]

1) \(\mathrm{CaSO}_{4}\)

2) \(\mathrm{BaCl}_{2}\)

3) \(\mathrm{NaCl}\)

4) Urea

104. Vapour pressure of dilute aqueous solution of glucose is \(750 \mathrm{~mm}\) of mercury at \(373 \mathrm{~K}\). The mole fraction of solute is [J\&K CET 2004]

\(\begin{array}{llll}1) & \frac{1}{76} & 2) & \frac{1}{7.6} \\ \text { 3) } & \frac{1}{38} & \text { 4) } & \frac{1}{10}\end{array}\)

105. The vapour pressure of water at

If \(18 \mathrm{~g}\) of glucose \(\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)\) is added to 178.2

\(\mathrm{g}\) of water at \(20^{\circ} \mathrm{C}\), the vapour pressure of the resulting solution will be [AIEEE 2008]

1) \(17.675 \mathrm{mmHg}\)

2) \(15.750 \mathrm{mmHg}\)

3) \(16.500 \mathrm{mmHg}\)

4) \(17.325 \mathrm{mmHg}\)

106. The empirical formula of a nonelectrolyte is \(\mathrm{CH}_{2} \mathrm{O}\). A solution containing \(3 \mathrm{~g}\) of the compound exerts the same osmotic pressure as that of \(0.05 \mathrm{M}\) glucose solution. The molecular formula of the compound is

[KCET 2011]

1)

\(\mathrm{CH}_{2} \mathrm{O}\)

2)

\(\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}_{2}\)

3)

\(\mathrm{C}_{4} \mathrm{H}_{8} \mathrm{O}_{4}\)

4)

\(\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}_{3}\)

107. Which of the following solutions will have the highest boiling point ? [J\&K CET 2004]

1) \(0.1 \mathrm{M} \mathrm{FeCl}_{3}\)

2) \(0.1 \mathrm{M} \mathrm{BaCl}\)

3) \(0.1 \mathrm{M} \mathrm{NaVl}\)

4) \(0.1 \mathrm{M}\) urea

108. The freezing point of water is depressed by \(0.37^{\circ} \mathrm{C}\) in a \(0.01 \mathrm{~mol} \mathrm{NaCl} \mathrm{solution.} \mathrm{The}\) freezing point of 0.02 molal solution of urea is depressed by [WB JEE 2008]

1) \(0.37^{\circ} \mathrm{C}\)

2) \(0.74^{\circ} \mathrm{C}\)

3) \(0.185^{\circ} \mathrm{C}\)

4) \(0^{\circ} \mathrm{C}\)

109. The increase in boiling point of a solution containing \(0.6 \mathrm{~g}\) urea in \(200 \mathrm{~g}\) water is \(0.50^{\circ} \mathrm{C}\). Find the molal elevation constant. [Guj CET 2009]

1) \(10 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\)

2) \(10 \mathrm{Kg} \mathrm{mol}^{-1}\)

3) \(10 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}\)

4) \(1.0 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\)

\(110.20 \mathrm{~g}\) of binary electrolyte (mol. wt. =100) are dissolved in \(500 \mathrm{~g}\) of water. The depression in freezing point of the solution is \(0.74^{\circ} \mathrm{C}\) ( \(k_{f}=1.86 \mathrm{Km}^{-1}\) ) the degree of ionisation of the electrolyte is [Manipal 2003]

1) \(0 \%\)

2) \(100 \%\)

3) \(75 \%\)

4) \(50 \%\)

111.A solution containing \(1.8 \mathrm{~g}\) of a compound (empirical formula \(\mathrm{CH}_{2} \mathrm{O}\) ) in \(40 \mathrm{~g}\) of water is observed to freeze at \(-0.465^{\circ} \mathrm{C}\). The molecular formula of the compound is \(\left(K_{f}\right.\) of water \(\left.=1.86 \mathrm{kgKmol}^{-1}\right)\)

[Kerala CEE

2011]

1) \(\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}_{2}\)

\(\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}_{3}\)

3) \(\mathrm{C}_{4} \mathrm{H}_{8} \mathrm{O}_{4}\)

4) \(\mathrm{C}_{5} \mathrm{H}_{10} \mathrm{O}_{5}\)

5)

\(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\)

112. A solution of sucrose (Molar mass \(=342\) \(\mathrm{g} / \mathrm{mol}\) ) is prepared by dissolving \(68.4 \mathrm{~g}\) of it per litre of solution, what is its osmotic pressure \(\left(\mathrm{R}=0.082 \mathrm{~L} \mathrm{~atm}^{-1} \mathrm{~mol}^{-1}\right)\) at \(273 \mathrm{~K}\) ? [BITSAT 2007]

1) \(3.92 \mathrm{~atm}\)

2) \(4.48 \mathrm{~atm}\)

3) \(5.92 \mathrm{~atm}\)

4) \(29.4 \mathrm{~atm}\)

113. The freezing point depression constant for water is \(1.86 \mathrm{~K} \mathrm{kgmol}^{-1}\). If \(45 \mathrm{~g}\) of ethylene glycol is mixed with \(600 \mathrm{~g}\) of water , the freezing point of the solution is [BCECE 2004]

1) \(2.2 \mathrm{~K}\)

2) \(270.95 \mathrm{~K}\)

3) \(273 \mathrm{~K}\)

4) \(275.35 \mathrm{~K}\)

114. In a 0.2 molal aqueous solution of a weak acid \(\mathrm{H} X\), the degree of ionisation is 0.3 Taking \(k_{f}\) for water as 1.85 , the freezing point of the solution will be nearest to [MP PET 2007]

\(1)^{-0.480^{\circ} \mathrm{C}}\)

2) \(-0.360^{\circ} \mathrm{C}\)

\(3)^{-0.260^{\circ} \mathrm{C}}\)

4) \(+0.480^{\circ} \mathrm{C}\)

115. For determination of molar mass of colloids, polymers and protein, which property is used?

[OJEE 2004] 

1) Diffusion pressure

2)Atmospheric pressure

3) Osmotic pressure

4) Turgor pressure

116. The relative lowering of vapour pressure of a dilute aqueous solution containing non-volatile solute is 0.0125 . The molality of the solution is about [Kerala CEE 2007]

1) 0.70

2) 0.50

3) 0.90

4) 0.80

5) 0.60

117. In a 0.2 molal aqueous solution of a weak acid \(\mathrm{H} X\), the degree of ionisation is 0.3 Taking \(k_{f}\) for water as 1.85 , the freezing point of the solution will be nearest to [J\&K CET 2007]

1) \(\mathrm{MeV}\)

2) Cal

3) \(\mathrm{Cm} / \mathrm{s}\)

4) Atm

118. Which of the following shows maximum depression in freezing point? [BCECE 2005] \(\begin{array}{ll}\text { 1) } \mathrm{K}_{2} \mathrm{SO}_{4} & \text { 2) } \mathrm{NaCl}\end{array}\)

3) Urea 4)glucose

119. A solution of \(4.5 \mathrm{~g}\) of a pure non-electrolyte in \(100 \mathrm{~g}\) of water was found to freeze at \(0.465^{\circ} \mathrm{C}\). The molecular weight of the solute closest to ( \(k_{f}=1.86\) ) [Kerala CEE 2003]

1) 135.0

2) 172.0

3) 90.0

4) 86.2

5) 180.0

120. Which of the following statement is true?

\section{[OJEE 2003]}

1) The relative

2) Passage of solute lowering of vapour molecules towards pressure of a solution side through solution is equal to semipermeable the mole fraction of membrane is the solute present in osmosis. the solution

3) The boiling point of

4) The boiling point of solution is always a liquid is the lower than the temperature at solvent. which its vapour pressure becomes equal to \(260 \mathrm{~mm}\).

121. Solution \(A\) contains \(7 \mathrm{~g} / \mathrm{L}\) of \(\mathrm{MgCl}_{2}\) and solution \(B\) contains \(7 \mathrm{~g} / \mathrm{L}\) of \(\mathrm{NaCl}\). At room temperature, the osmotic pressure of [DCE 2005]

1) Solution \(A\) is greater 2) Both have same than \(B\) osmotic pressure 3) Solution \(B\) is greater 4)Cannot be determine than \(A\)

122. In an osmotic pressure measurement experiment, a \(5 \%\) solution of compound ' \(X\) ' is found to be isotonic with a \(2 \%\) acetic acid solution. The gram molecular mass of ' \(X\) ' is [AMU 2005]

1) 24

2) 60

3) 150

4) 300

123. A 5.25\% solution of a substance is isotonic with a \(1.5 \%\) solution of urea (molar mass \(=60\) gmol \(^{-1}\) ) in the same solvent. If the densities of both the solutions are assumed to be equal to \(1.0 \mathrm{~g} \mathrm{~cm}^{-3}\), molarmass of the substance will be [AIEEE 2007]

1) \(90.0 \mathrm{~g} \mathrm{~mol}^{-1}\)

2) \(115.0 \mathrm{~g} \mathrm{~mol}^{-1}\)

3) \(105.0 \mathrm{~g} \mathrm{~mol}^{-1}\)

4) \(210.0 \mathrm{~g} \mathrm{~mol}^{-1}\)

124. A solution of sucrose (Molar mass \(=342\)

\(\mathrm{g} / \mathrm{mol}\) ) is prepared by dissolving \(68.4 \mathrm{~g}\) of it per litre of solution, what is its osmotic pressure \(\left(\mathrm{R}=0.082 \mathrm{~L} \mathrm{~atm}^{-1} \mathrm{~mol}^{-1}\right)\) at \(273 \mathrm{~K}\) ? [UP SEE 2007]

1) \(0.01 \mathrm{M} \mathrm{Na}_{2} \mathrm{SO}_{4}\)

2) \(0.01 \mathrm{M} \mathrm{KNO}_{3}\)

3) \(0.015 \mathrm{M}\) urea

4) \(0.015 \mathrm{M}\) glucose

125. Solutions \(A, B, C\) and \(D\) are respectively \(0.1 \mathrm{M}\) glucose, \(0.05 \mathrm{M} \mathrm{NaCl}, 0.05 \mathrm{M} \mathrm{BaCl}_{2}\) and \(0.1 \mathrm{M}\) \(\mathrm{AlCl}_{3}\). Which one of the following pairs is isotonic? [MHT CET 2008]

1) \(A\) and \(B\)

2) \(B\) and \(C\)

3) \(A\) and \(D\)

4) \(A\) and \(C\)

126. The relationship between the values of osmotic pressure of \(0.1 \mathrm{M}\) solution of \(\mathrm{KNO}_{3}\left(p_{1}\right)\) and \(\mathrm{CH}_{3} \mathrm{COOH}\left(p_{2}\right)\) is [DCE 2004]

1) \(\frac{p_{1}}{p_{1}+p_{2}}=\frac{p_{2}}{p_{1}+p_{2}}\)

2) \(p_{1}>p_{2}\)

3)

\(p_{2}>p_{1}\)

4)

\(p_{1}=p_{2}\)

127. At \(25^{\circ} \mathrm{C}\) a \(5 \%\) aqueous solution of glucose (molecular weight \(=180 \mathrm{~g} \mathrm{~mol}^{-1}\) ) is isotonic with \(2 \%\) aqueous solution containing an unknown solute. What is the molecular weight of the unknown solute. [Kerala CEE 2011]

1) 60

2) 80

3) 72

4) 63

5) 98 128. Relative lowering of vapour pressure of a dilute solution is 0.2 . What is the mole fraction of the non-volatile solute? [Guj CET 2006,J\&K CET

\section{6]}

1) 0.8

2) 0.5

3) 0.3

4) 0.2

129. If a solution containing \(0.072 \mathrm{~g}\) atm of sulphur in \(100 \mathrm{~g}\) of a solvent \(\left(k_{f}=7.0\right)\) gave a freezing point depression of \(0.84^{\circ} \mathrm{C}\), the molecular formula of sulphur in the solution is

[Jamia Millia Islamia 2006]

\(\begin{array}{cccc}1) & S_{6} & 2) & S_{7} \\ \text { 3) } & S_{8} & 4) & S_{9}\end{array}\)

130. Which of the following solutions will have the highest boiling point? [J\&K CET 2004]

1) Camphor

2) Naphthalene

3) Benzene

4) Water

131. By dissolving \(5 \mathrm{~g}\) substance in \(50 \mathrm{~g}\) of water, the decrease in freezing point is \(1.2^{\circ} \mathrm{C}\). The gram molal depression is \(1.85^{\circ} \mathrm{C}\). The molecular weight of substance is [WB JEE 2006]

1) 105.4

2) 118.2

3) 137.2

4) 154.2

132. Which of the following solutions will have highest boiling point [MHT CET 2008]

1) \(0.1 \mathrm{M} \mathrm{FeCl}_{3}\)

2) \(0.1 \mathrm{M} \mathrm{BaCl}\)

3) \(0.1 \mathrm{M} \mathrm{NaCl}\)


133. Elevation in boiling point was \(0.52^{\circ} \mathrm{C}\) when \(6 \mathrm{~g}\) of a compound was dissolved in \(100 \mathrm{~g}\) of water. Molecular weight of \(X\) is \(\left(k_{b} o f\right.\) water is \(5.2^{\circ} \mathrm{C}\) per \(100 \mathrm{~g}\) water ) [BCECE 2003]

1) 120

2) 60

3) 600

4) 180

134. The freezing point of water is depressed by \(0.37^{\circ} \mathrm{C}\) in a \(0.01 \mathrm{~mol} \mathrm{NaCl}\) solution. The freezing point of 0.02 molal solution of urea is depressed by [BCECE 2008]

1) Hypotonic

2) Isotonic

3) Equimolar

4) Hypertonic

135. Which of the following is incorrect? [UP SEE 2005]

1) \(0.1 \mathrm{~m}\) sucrose

2) \(0.1 \mathrm{~m}\) urea

3) \(0.1 \mathrm{~m}\) ethanol

4) \(0.1 \mathrm{~m}\) glucose

136.18 g of glucose \(\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)\) is added to \(178.2 \mathrm{~g}\) of water. the vapour pressure of water for this aqueous solution at \(100^{\circ} \mathrm{C}\) is [AIEEE 2006]

1) 759.00 torr

2) 7.60 torr

3) 76.00 torr

4) 752.40 torr

137. What is the freezing point of a solution containing \(8.1 \mathrm{~g} \mathrm{HBr}\) in \(100 \mathrm{~g}\) water assuming the acid to be \(90 \%\) ionised? \(\left(k_{f}\right.\) for \(\left.w t .=1.86 \mathrm{~K} \mathrm{~mol}^{-1}\right)\) [JCECE 2010]

1) \(0.85^{\circ} \mathrm{C}\)

\(2)^{-3.53^{\circ} C}\)

3)

\(0^{\circ} C\)

4) \(-0.35^{\circ} C\)

138. Which of the following solution highest boiling point? [AMU 2003]

1) \(0.1 \mathrm{M}\) urea

2) \(0.1 \mathrm{M}\) sucrose

3) \(0.1 \mathrm{M} \mathrm{NaNO}_{3}\)

4) \(0.1 \mathrm{M} \mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\)

139. If the elevation in boiling point of a solution of \(10 \mathrm{~g}\) of solute (mol. wt. \(=100 \mathrm{~g}\) of water is \(\Delta T_{b}\), the ebullioscopic constant of water is

\section{[Kerala CEE 2007]}

1) 10

2) \(100 \Delta T_{b}\)

3)

\(\Delta T_{b}\)

4) \(\frac{\Delta T_{b}}{10}\)

5) \(10 T_{b}\)

140. The statement "the relative lowering of the vapour pressure is equal to th ratio ot moles of the solute to the total number of the moles in the solution" refers to [Kerala CEE 2004]

1) Hess's law

2) Dalton's law

3) Raoult's law

4) Charles'law

5) Boyle's law

141.The relative lowering of vapour pressure of an aqueous solution containing non-volatile solute is 0.0125 . The molality of the solution is [OJEE 2008]

1) Vapour pressure

2) Osmotic pressure

3)Boiling point

4) Freezing point

142. The vapour pressure of pure liquid is \(1.2 \mathrm{~atm}\). When a non-volatile substance \(B\) is mixed in \(A\), then its vapour pressure becomes \(0.6 \mathrm{~atm}\). The mole fraction of \(B\) in the solution is [MP PET 2003]

1) 0.15

2) 0.25

3) 0.50

4) 0.75 143. Equimolar solution in the same solvent have

\section{[AIEEE 2005]}

1) Different boiling and 2) Same boiling and different freezing same freezing points points

3) Same freezing point 4) Same boiling point but different boiling but different freezing point point

144. The vapour pressure will be lowest of [WB JEE 2006]

1) Hypertonic solution 2) Hypotonic solution

3) Isotonic solution 4) None of the above

145. Osmotic pressure of \(0.4 \%\) urea solution is 1.60 atm and that of \(3.42 \%\) cane sugar is \(2.46 \mathrm{~atm}\). When the above two solutions are mixed, the osmotic pressure of the resulting solution is

[UP SEE 2006]

1) \(0.82 \mathrm{~atm}\)

2) \(2.46 \mathrm{~atm}\)

3) \(1.64 \mathrm{~atm}\)

4) \(4.10 \mathrm{~atm}\)

146. Which of the following is not a colligative property? [UP SEE 2009]

1) Optical activity

2) Osmotic pressure

3) Depression of

4) Elevation of boiling freezing point point

147. The difference between the boiling point and freezing point of an aqueous solution containing sucrose \(\left(\mathrm{mol} \mathrm{wt} .=342 \mathrm{gmol}^{-1}\right)\) in \(100 \mathrm{~g}\) of water is \(105.0^{\circ} \mathrm{C}\). If \(K_{f}\) and \(K_{b}\) of water are 1.86 and \(0.51 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\) respectively, the weight of sucrose in the solution is about

\section{[Manipal 2009]}

1) 1 M solution of

2) 0.05 M solution of glucose glucose

3) \(6 \%\) solution of

4) \(25 \%\) solution of glucose glucose

148. If \(0.1 \mathrm{M}\) solutions of each electrolyte are taken and if all electrolytes are completely dissociated, then whose boiling point will be highest? [Indraprastha CET 2009]

1) Glucose

2) \(\mathrm{KCl}\)

3) \(\mathrm{BaCl}_{2}\)

4) \(\mathrm{K}_{2}\left[F e(C N)_{6}\right]\)

149. The movement of solvent molecules through a semipermeable membrane is called [Manipal 2005]

1) Electrolysis

2) Electrophoresis

3) Osmosis

4) Cataphoresis

150. When \(25 \mathrm{~g}\) of a non-volatile solute is dissolved in \(100 \mathrm{~g}\) of water, the vapour pressure is lowered by \(2.25 \times 10^{-1} \mathrm{~mm}\). If the vapour pressure of water at \(20^{\circ} \mathrm{C}\) is \(17.5 \mathrm{~mm}\), what is the molecular weight of the solute? [BITSAT

\section{8]}

1) 206

2) 302

3) 350

4) 276

151.At a constant temperature, which of the following aqueous solutions will have the maximum vapour pressure?

(Mol. wt NaCl \(=58.5, \mathrm{H}_{2} \mathrm{SO}_{4}=98.0 \mathrm{~g} . \mathrm{mol}^{-1}\) )

[Guj CET 2010]

1) 1 molal \(\mathrm{NaCl}(a q) \quad\) 2) 1 molar \(\mathrm{NaCl}(a q)\)

3) 1 molal \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)\) 4) 1 molar \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)\)

152. The osmotic pressure of 0.2 molar solution of


[MP PET 2005]

1) \(4.92 \mathrm{~atm}\)

2) 1 atm

3) \(0.2 \mathrm{~atm}\)

4) \(27 \mathrm{~atm}\)

153. The osmotic pressure (At27 \({ }^{\circ} \mathrm{C}\) ) of an aqueous solution (200 mL) containing \(6 \mathrm{~g}\) of a protein is


molecular weight of protein is

[UP SEE 2008]

1) \(7.2 \times 10^{5}\)

\(2)^{3.6} 6 \times 10^{5}\)

3) \(1.8 \times 10^{5}\)

4) \(1.0 \times 10^{5}\)

154. For dilute solution Raoult's law states that [MP PET 2004]

1) The relative

2) The lowering of lowering of vapour vapour pressure is pressure is equal to equal to the mole mole fraction of fraction of solute solute

3) The vapour pressure 4) The relative lowering of the solution is of vapour pressure is equal to mole proportional to fraction of the amount of solute in solvent solution

155. What is the freezing point of a solution containing \(8.1 \mathrm{~g} \mathrm{HBr}\) in \(100 \mathrm{~g}\) water assuming the acid to be \(90 \%\) ionised? ( \(k_{f}\) forwater \(=1.86 \mathrm{Kmol}^{-1}\) ) [DCE 2003]

1) \(0.85^{\circ} \mathrm{C}\)

2) \(-3.53^{\circ} \mathrm{C}\)

3) \(0^{\circ} \mathrm{C}\)

4) \(-0.35^{\circ} \mathrm{C}\)

156. On adding a solute to a solvent having vapour pressure \(0.80 \mathrm{~atm}\) vapour pressure reduces to \(0.60 \mathrm{~atm}\). Mole fraction of solute is [UP SEE 2003] 

1) 0.25

2) 0.75

3) 0.50

4) 0.33

157. \(\operatorname{At} 25^{\circ} \mathrm{C}\), the highest osmotic pressure is exhibited by \(0.1 \mathrm{M}\) solution of [Manipal 2010]

1) Urea

2) Glucose

3) \(\mathrm{KCl}\)

4) \(\mathrm{CaCl}_{2}\)

158. The difference between the boiling point and freezing point of an aqueous solution containing sucrose \(\left(\mathrm{mol} \mathrm{wt} .=342 \mathrm{gmol}^{-1}\right)\) in \(100 \mathrm{~g}\) of water is \(105.0^{\circ} \mathrm{C}\). If \(K_{f}\) and \(K_{b}\) of water are 1.86 and \(0.51 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\) respectively, the weight of sucrose in the solution is about

[Kerala CEE 2009]

1) \(34.2 \mathrm{~g}\)

2) \(342 \mathrm{~g}\)

3) \(7.2 \mathrm{~g}\)

4) \(72 \mathrm{~g}\)

5) \(68.4 \mathrm{~g}\)

159. The freezing point of equimolal aqueous solution will be highest for [J\&K CET 2003]

1) \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3} \mathrm{Cl}\)

2) \(\mathrm{La}\left(\mathrm{NO}_{3}\right)_{3}\)

3)

\(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\)

4)

\(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\)

160. The empirical formula of a non-electrolyte is \(\mathrm{CH}_{2} \mathrm{O}\). A solution containing \(6 \mathrm{~g}\) of the compound exerts the same osmotic pressure as that of \(0.05 \mathrm{M}\) glucose solution at the same temperature. The molecular formula of the compound is [KCET 2010]

1)

\(\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}_{2}\)

2)

\(\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}_{3}\)

3)

\(\mathrm{C}_{5} \mathrm{H}_{10} \mathrm{O}_{5}\)

4)

\(\mathrm{C}_{4} \mathrm{H}_{5} \mathrm{O}_{4}\)

161.The relative lowering of vapour pressure of a dilute aqueous solution containing non-volatile solute is 0.0125 . The molality of the solution is about [Manipal 2010]

1) 0.70

2) 0.50

3) 0.90

4) 0.80

162. After adding a solute freezing point of solution decreases to -0.186. Calculate [OJEE 2004]

1) 0.512

2) 0.0512

3) 1.86

4) 0.0186

163. A solution containing \(4 \mathrm{~g}\) of polyvinyl chloride polymer in one litre of dioxane was found to have an osmotic pressure of \(4.1 \times 10^{-4}\) atm at \(27^{\circ} \mathrm{C}\). The approximate molecular weight of the polymer is [J\&K CET 2008]

1) \(1.5 \times 10^{3}\)

2) \(2.4 \times 10^{5}\)

3) \(1.0 \times 10^{4}\)

\(4)^{2 \times 10^{12}}\)

164. Ethylene glycol is used as an antifreeze in a cold climate. Mass of ethylene glycol which should be added to \(4 \mathrm{~kg}\) of water to prevent it from freezing at \(-6^{\circ} C\) will be ( \(K_{f}\) for water \(=1.86 \mathrm{Kkg} \mathrm{mol}^{-1}\). and molar mass of ethylene glycol \(=62 \mathrm{gmol}^{-1}\) ) [AIEEE 2011]

1) \(804.32 \mathrm{~g}\)

2) \(204.30 \mathrm{~g}\)

3) \(400.00 \mathrm{~g}\)

4) \(304.60 \mathrm{~g}\)

165. Colligative properties of a solution depends upon [Punjab CET 2010]

1) Nature of both

2) Nature of solute only solvent and solute

3) Number of solvent particles

4) The number of solute particles

166. The relative lowering of vapour pressure of an aqueous solution containing non-volatile solute is 0.0125 . The molality of the solution is

[Kerala CEE 2008]

1) 0.70

2) 0.50

3) 0.60

4) 0.80

5) 0.40

167. \(\operatorname{At} 25^{\circ} \mathrm{C}\), the highest osmotic pressure is exhibited by \(0.1 \mathrm{M}\) solution of [RPET 2010]

1)Decinormal

2) Decinormal barium aluminium sulphate chloride

3) Decinormal sodium

4)A solution obtained chloride by mixing equal volumes of (b) and (c) and filtering

168. Which is not a colligative property in the following? [MP PET 2008]

1) pH ofa buffer

2) Boiling point solution elevation

3) Freezing point

4) Vapour pressure depression lowering

169. Choose the correct statement.

When concentration of a salt solution is increased [Guj CET 2011]

1)Boiling point increases while vapour pressure decreases.

3) Freezing point decreases while 2) Boiling point decreases while vapour pressure increases.

4) Freezing point increases while vapour pressure

vapour pressure

increases.

decreases.

170. Which of the following is incorrect? [J\&K CET

\section{5]}

1) Relative lowering of 2)The relative lowering vapour pressure is of vapour pressure is independent of the a colligative solute and the property. solvent.

3) Vapour pressure of a 4)The relative lowering solution is lower of vapour pressure is than the vapour directly proportional pressure of the to the original solvent. pressure.

171. Osmotic pressure of a solution at a given temperature [UP SEE 2008]

1) Increases with

2) Decreases with concentration concentration

3) Remains same

4) Initially increases and then decreases

172. What is the amount of urea dissolved per litre if its aqueous solution is isotonic with \(10 \%\) cane sugar solution? (mol.wt.of urea \(=60\) )

[DCE 2008]

1) \(200 \mathrm{~g} / \mathrm{L}\)

2) \(19.2 \mathrm{~g} / \mathrm{L}\)

3) \(17.54 \mathrm{~g} / \mathrm{L}\)

4) \(16.7 \mathrm{~g} / \mathrm{L}\)

173. Which one is a colligative property? [OJEE 2007]

1)Boiling point

2) Vapour pressure

3)Osmotic pressure

4) Freezing point

174. For an aqueous solution, freezing point is \(-0.186^{\circ} \mathrm{C}\). Elevation of the boiling point of the same solution is \(\left(k_{f}=1.86^{\circ} \mathrm{mol}^{-1} \mathrm{~kg}\right.\) and [Jamia Millia Islamia 2005]

1) \(0.186^{\circ}\)

2) \(0.0512^{\circ}\)

\(3^{1.86^{\circ}}\)

\(4)^{5.12^{\circ}}\)

175. Which one is a colligative property? [Jamia

\section{Millia Islamia 2007]}

1) Raoult's law states

The osmotic that the vapour pressure of a component over a solution is proportional to its pressure ( \(\pi\) )of a solution is given by

2) the equation \(\pi=\) \(M R T\), where, \(M\) is the molarity of the mole fraction solution The correct order of

3) osmotic pressure for

4) Two sucrose \(0.01 \mathrm{M}\) aqueous solutions of same molality prepared in solution of each

different solvents

compound is will have the same

\(\mathrm{BaCl}_{2}>\mathrm{KCl}>\mathrm{CH}_{3} 1\)

freezing point

sucrose depression

176. A 5\% solution of cane sugar (molar mass 342) is isotonic with \(1 \%\) of a solution of an unknown solute. The molar mass of unknown solute in \(\mathrm{g} / \mathrm{mol}\) is [AIEEE 2011]

1) 136.2

2) 171.2

3) 68.4

4) 34.2

177. If \(0.15 \mathrm{~g}\) of a solute, dissolved in \(15 \mathrm{~g}\) of solvent, is boiled at a temperature higher by \(0.216^{\circ} \mathrm{C}\) than that of the pure solvent. The molecular weight of the substance (molal elevation constant for the solvent is \(2.16^{\circ} \mathrm{C}\) ) is [MHT CET 2003]

1) 100

2) 10.1

3) 10

4) 1.001

178. The statement "the relative lowering of the vapour pressure is equal to th ratio ot moles of the solute to the total number of the moles in the solution" refers to [Kerala CEE 2004]

1) Decrease the

2)Only decrease the freezing point of freezing point of water in the winter water and increase the boiling point of water in the summer

3)Only increase the

4)Be used for cleaning boiling point of the radiator in a car water

5) Prevent corrosion of automobile parts

179.An 1\% solution of \(\mathrm{KCl}\) (I), \(\mathrm{NaCl}\) (II), \(\mathrm{BaCl}_{2}\) (III) and urea (IV) have their osmotic pressure at the same temperature in the ascending order (molar masses of \(\mathrm{NaCl}, \mathrm{KCl}, \mathrm{BaCl}_{2}\) and urea are respectively \(58.5,74.5,208.4\) and \(60 \mathrm{~g} \mathrm{~mol}^{-1}\) ). Assume \(100 \%\) ionisation of the electrolytes at this temperature [Kerala CEE 2009]

1) I \(<\) III \(<\) II \(<\) IV

2) \(\mathrm{III}<\) I \(<\) II \(<\) IV

3) I \(<\) II \(<\) III \(<\) IV

4) I \(<\) III \(<\) IV \(<\) II

5) III \(<\) IV \(<\) I \(<\) II

180.The molar freezing point constant for water is

\(1.86^{\circ} \mathrm{C} / \mathrm{mol}\). If \(342 \mathrm{~g}\) of cane sugar (

\(C_{12} \mathrm{H}_{22} \mathrm{O}_{11}\) ) is dissolved in \(1000 \mathrm{~g}\) of water, the solution will freeze at

1) \(-1.86^{\circ} \mathrm{C}\)

2) \(1.86^{\circ} \mathrm{C}\)

[Manipal 2005] 

3) \(-3.92^{\circ} \mathrm{C}\)

4) \(2.42^{\circ} \mathrm{C}\)

181. On adding \(1 \mathrm{~g}\) arsenic to \(80 \mathrm{~g}\) benzene, the freezing point of benzene is lowered by 0. \(19^{\circ} \mathrm{C}\). The formula of arsenic is [UP SEE 2008]

1) As

2)

\(A s_{2}\)

3)

\(A s_{3}\)

4)

\(A s_{4}\)

182. Which is a colligative property ? [MP PET

\section{6]}

1) Osmotic pressure

2) Free energy

3) Heat of vaporisation

4) Change in pressure

183. Depression in freezing point is \(6 \mathrm{~K}\) for \(\mathrm{NaCl}\) solution if \(k_{f}\) for water is \(1.86 \mathrm{~K} / \mathrm{kg} \mathrm{mol}\), amount of \(\mathrm{NaCl}\) dissolved in \(1 \mathrm{~kg}\) water is [DCE 2006]

1) 3.42

2) 1.62

3) 3.24

4) 1.71

184. Which has minimum osmotic pressure? [DCE

\section{5]}

1) \(200 \mathrm{~mL}\) of \(2 \mathrm{M} \mathrm{NaCl}\)

2) \(200 \mathrm{~mL}\) of \(2 \mathrm{M}\) solution glucose solution

3) \(200 \mathrm{~mL}\) of \(2 \mathrm{M}\) urea

4) All have same solution osmotic pressure

185. Calculate the molal depression constant of a solvent which has freezing point \(16.6^{\circ} \mathrm{C}\) and latent heat of fusion \(180.75 \mathrm{Jg}^{-1}\). [OJEE 2005]

1) 2.68

2) 3.86

3) 4.68

4) 2.86

186. The freezing point of the 0.05 molal solution of non-electrolyte in water is [MHT CET 2006]

1) \(-0.093^{\circ} \mathrm{C}\)

2) \(1.86^{\circ} \mathrm{C}\)

3) \(0.93^{\circ} \mathrm{C}\)

4) \(0.093^{\circ} \mathrm{C}\)

187. Consider the following aqueous solutions and assume \(100 \%\) ionisation in electrolytes

1. \(0.1 \mathrm{~m}\) urea

2. \(\quad 0.04 \mathrm{~m}\)

3. \(\quad 0.05 \mathrm{~m}\)

4. \(\quad 0.005 \mathrm{~m} \mathrm{NaCl}\)

The correct statement regarding the above solution is [Guj CET 2008]

1) Freezing point will

2) Freezing point will be lowest for be highest for solution I solution IV 3) Boiling point will be 4) Vapour pressure will highest for solution be highest for IV solution II

188. The vapour pressure of benzene at a certain temperature is \(640 \mathrm{~mm}\) of \(\mathrm{Hg}\). A non-volatile and non-electrolyte solid weighing \(2.175 \mathrm{~g}\) is added to \(39.08 \mathrm{~g}\) of benzene. If the vapour pressure of the solution is \(600 \mathrm{~mm}\) of \(\mathrm{Hg}\), what is the molecular weight of solid substance?

\section{[MHT CET 2008]}

1) 49.50

2) 59.60

3) 69.60

4) 79.82

189. The order of osmotic pressure of isomolar solution of \(\mathrm{BaCl}_{2}, \mathrm{NaCl}\) and sucrose is [MP PET 2003]

1) \(\mathrm{BaCl}_{2}\)

\(>\mathrm{NaCl}>\) sucrose

2) \(\mathrm{NaCl}>\mathrm{BaCl}_{2}>\)

Sucrose \(>\mathrm{NaCl}>\)

3) \(\mathrm{BaCl}_{2}\)

\(\mathrm{BaCl}_{2}\)

190. The mass of glucose that should be dissolved in \(50 \mathrm{~g}\) of water in order to produce the same lowering of vapour pressure as is produced by dissolving \(1 \mathrm{~g}\) of urea in the same quantity of water is [Jamia Millia Islamia 2008]

1) \(1 \mathrm{~g}\)

2) \(3 \mathrm{~g}\)

3) \(6 \mathrm{~g}\)

4) \(18 \mathrm{~g}\)

191. The vapour pressure of pure liquid \(A\) is 0.80 atm. When a non-volatile \(B\) is added to \(A\) its vapour pressure drops to \(0.60 \mathrm{~atm}\). The mole fraction of \(B\) in the solution is [AMU

2008,EAMCET 2008,UP SEE 2008]

1) 0.125

2) 0.25

3) 0.5

4) 0.75

192. Maximum lowering of vapour pressure is observed in the case of [J\&K CET 2008]

1) \(0.1 \mathrm{M}\) glucose

2) \(0.1 \mathrm{M} \mathrm{Bacl}_{2}\)

3) \(0.1 \mathrm{M} \mathrm{MgSO}_{4}\)

4) \(0.1 \mathrm{NaCl}\)

193. The freezing point of \(1 \%\) solution of lead nitrate in water will be [Manipal 2006]

1) \(2^{\circ} \mathrm{C}\)

2) \({ }^{\circ} \mathrm{C}\)

3) \(0^{\circ} \mathrm{C}\)

4)Below \(0^{\circ} \mathrm{C}\)

194.At temperature \(327^{\circ} \mathrm{C}\) and concentration \(C\) osmotic pressure of a solution is \(p\), the same solutions at concentration \(C / 2\) and a temperature \(427^{\circ} \mathrm{C}\) shows osmotic pressure 2 atm, value of \(p\) will be [DCE 2007] 

1) \(\frac{12}{7}\)

2) \(\frac{24}{7}\)

3) \(\frac{6}{5}\)

4) \(\frac{5}{6}\)

195. The relative lowering of vapour pressure of an aqueous solution containing non-volatile solute is 0.0125 . The molality of the solution is

[OJEE 2008]

1) \(0.1 \mathrm{M} \mathrm{NaCl}\)

2) \(0.1 \mathrm{M} \mathrm{BaCl}\)

3) \(0.1 \mathrm{M}\) sucrose

4) \(0.1 \mathrm{M} \mathrm{KCl}\)

196. The vapour pressure will be lowest of [WB JEE 2006]

1) \(0.1 \mathrm{M}\) sugar solution

2) \(0.1 \mathrm{M} \mathrm{KCl}\) solution

3) \(0.1 \mathrm{MCu}\left(\mathrm{NO}_{3}\right)_{2}\) \(0.1 \mathrm{M} \mathrm{AgNO}_{3}\) solution soution

197. In countries nearer to polar region, the roads are sprinkled with \(\mathrm{CaCl}_{2}\). This is [Manipal 2009]

1) To minimise the

2) To minimise the wear and tear of the snow fall roads

3)To minimise \(\quad\) 4)To minimise the pollution accumulation of dust on the road

198. A \(5 \%\) solution of sugarcane (mol. wt. \(=342\) ) is isotonic with \(1 \%\) solution of \(X\) under similar conditions. The molecular weight of \(X\) is [DCE 2009]

1) 136.2

2) 689.4

3) 34.2

4) 171.2

199. The amount of urea dissolved in \(500 \mathrm{cc}\) of water \(\left(K_{f}=1.86^{\circ} \mathrm{C}\right)\) to produce a depression of \(0.186^{\circ} \mathrm{C}\) in the freezing point is [Manipal

2006]

1) \(9 \mathrm{~g}\)

2) \(6 \mathrm{~g}\)

3) \(3 \mathrm{~g}\)

4) \(0.3 \mathrm{~g}\)

200. Which has the minimum freezing point?

[Jamia Millia Islamia 2006]

1) One molal \(\mathrm{NaCl}\) aqueous solution 2) One molal \(\mathrm{CaCl}_{2}\) aqueous solution

3) One molal \(\mathrm{KCl}\)

4) One molal urea aqueous solution aqueous solution